Estimate of condensation rate

We want to estimate how quickly a layer of condensation would form on our sample, and how much of the incoming light will be absorbed by this layer. The estimate below is very crude, but serves as a starting point.

Known quantities

Pressure p = 1e-3 Pa (or 1e-5mbar)

Temperature T = 293 K

Volume V = 0.014 m³ (estimated volume of vacuum chamber only)

Gas constant R = 8.314 Jmol^-1K^-1

Avogadro's constant N_A = 6.022e23 mol^-1

Boltzmann constant k_B = 1.380649e-23 JK^-1

With the ideal gas law, we calculate the amount of air in the vacuum chamber to be 5.75e-9 mol. At sea level we will assume the atmosphere contains 2% water vapour. So, we get n = 0.02*5.75e-9 = 1.15e-10 mol water in our system. The molar mass M of H₂O is 18 gmol^-1.

Estimate of light absorption due to water condensation

For the velocity v of the water molecules, we use v = sqrt(3*R*T/M) = 636 ms^-1 (most probable velocity) and calculate the collision rate per second per square meter as r = 0.5*n*N_A*v/V = 1.57e18 s^-1m^-2.

Now let's calculate how many molecules there will be in a monolayer of water covering our 3cm x 3cm sample. A cm³ of water has N_A/18 water molecules, taking the cube root of that gives us 32222517 layers of molecules, with each 32222517*32222517 molecules. We have 9 cm², so in total 9.3e15 molecules would go into a single layer.

Using the collision rate and assuming that all molecules that hit the sample will neatly arrange themselves into a single layer as long as there is space, we calculate that it takes 9.3e15/(r*0.03*0.03) = 6.6 s to form a single layer of water on our sample.

Now, a single layer has a thickness of 1/32222517 cm with the same argument as before. So, after 60 seconds we will have a 2.83e-7 cm thick layer of water on our sample. Now, with the Lambert-Beer law, we calculate that at 125 nm, where the absorption coefficient* is 1.978e5 cm^-1, we have I=100*exp(-1.978e5*2.83e-7) = 94.6% of our light remains and so about 6% is absorbed. At 175 nm the absorption coefficient* is 1.705e1 and therefore 99.999% of our light remains.

So, how long would it take to lose half our intensity? For 125 nm it will take ~750s (corresponding to an 3.5e-6 cm thick layer of water) and for 175 nm it will take ~100 days (corresponding to a 0.4mm thick layer of water).

Worst case scenario

Now, let's compare the above estimate to an absolute worst case scenario. Let's assume all the air in the vacuum chamber is actually water vapour. So, we have 5.75e-9 mol of water. We stick all this water in layers on our sample: so there is nothing left in the rest of the vacuum chamber. Each layer would have again 9.3e15 molecules, which means we get 5.79e-9*N_A/9.3e15 layers. Each layer is 1/32222517 cm, giving us a water layer of 5.79e-9*N_A/(9.3e15*32222517) = 1.15e-8 cm thick. Note that this is less than the layer thickness we calculated before after 60 s. Meaning that the above calculation is actually worse than the absolute worst case. Of course, we assume here there is no additional outgassing which could make the answer even worse.

*Absorption coefficients taken from S. G. Warren, "Optical constants of ice from the ultraviolet to the microwave," Appl. Opt., 23, 1026--1225, (1984).

This data is based on the revised 1995 data of Warren. It was revised from the original data in the 1984 paper to account for misinterpretations of data by others. It also includes new data from Kou.

It is for ice, but for water I cannot find the appropriate values for the wavelengths we are interested in. I see other people use this data as well as if it was for water.